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Organic & Inorganic Chemistry > ATOMIC STRUCTURE > Flashcards

ATOMIC STRUCTURE Flashcards

1
Q

Atom came from the Greek word ___ meaning “uncut” or “indivisible”

A

atomos

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2
Q

A particle of matter that uniquely defines a chemical element.

A

Atom

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3
Q

Mention the years (6) on the evolution of atomic theory.

A

5th century BC- 1803-1897-1911-1913-1926

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4
Q

Mention the six models with their creators on the evolution of atomic theory in order.

A

Atomism (Democritus)
Solid Sphere Model (John Dalton)
Plum Pudding Model (J.J. Thomson)
Nuclear Model (Ernest Rutherford)
Planetary Model (Niels Bohr)
Quantum Model (Erwin Schrodinger)

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5
Q

He stated that it is impossible to pinpoint or determine accurately both momentum and position of electron simultaneously. Who said it and what is this principle?

A

Weiner Heisenberg (UNCERTAINTY PRINCIPLE)

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6
Q

Involves the small nucleus and the three elementary particles called the protons, electrons, and neutrons.

A

Modern Atomic Theory

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7
Q

contains the protons and the neutrons surrounded by an electron cloud.

A

Nucleus

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8
Q

___ discovered the electron using the ___ and he named his model the PLUM PUDDING MODEL

A

Joseph Jon Thomson - cathode ray tube

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9
Q

Discovered protons using the CANAL RAY TUBE

A

Eugen Goldstein

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10
Q

studied the alpha particles in ___, which lead to the discovery of neutron

A

Sir James Chadwick- beryllium

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11
Q

____ perceived the atom as a miniature solar system and used the ____ leading to the discovery of the nucleus

A

Ernest Rutherford - alpha scattering apparatus

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12
Q

+2, stopped by a thin sheet of paper

A

Alpha (Rutherford’s Experiment)

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13
Q

-1, stopped by a 1 cm thick of aluminum foil

No charge, stopped by lead (neutron)

A

Beta

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14
Q

What is the specific electrical charge of electron (-1)?

A

-1.602 x 10^-19

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15
Q

What is the specific electrical charge of proton (+1)?

A

+ 1.602 x 10^-19

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16
Q

What is the electrical charge of neutron?

A

0

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17
Q

What is another term for Mass number?

A

Massenzahl

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18
Q

What is another term for Atomic number?

A

Atomzahl

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19
Q

What are the 4 ways to separate isotopes? (TCEF)

A

Thermal Diffusion, Centrifugation, Electrolysis, Fractional Distillation

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20
Q
  • Are artificial radioactive isotopes
  • Are prepared by the bombardment of naturally occurring at
A

Radioisotopes

21
Q

Who discovered radioisotopes?

A

Irene and Frederic Joliot Curie

22
Q

Name of the protons and neutrons inside the nucleus

A

Nucleons

23
Q

Electrically charged atoms (positive and negative ions)

A

Ions

24
Q

Atoms having different atomic weights or mass but of the same atomic number

A

Isotopes

25
Q

Who discovered isotopes

A

Frederick Soddy

26
Q

Orderly distribution of electrons among the orbitals of an atom

A

Electron Configuration

27
Q

What do you call the s,p,d,f (2,6,10,14) format?

A

Mnemonic device

28
Q

Lowest, most stable energy state of the atom

A

Ground State

29
Q

Electrons are added one at a time to the lowest energy orbitals

A

Aufbau principle

30
Q

Aufbau principle came from the German word “___” meaning “TO BUILD UP”

A

aufbaue

31
Q

No two electrons can occupy the same quantum state simultaneously in an atom
a. An orbital can hold a maximum of 2 electrons
b. The electrons can occupy the same orbital if they spin in opposite direction
 clockwise (upward arrow)
 counterclockwise (downward arrow)

A

Pauli Exclusion Principle

32
Q
  • When electrons occupy orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with parallel spins
  • Second electrons then add to each orbital pairing the spins of the first electrons
A

Hund’s Rule

33
Q

*Electrons in the outermost energy level
*Determines the chemical properties of elements

A

Valence Electron

34
Q

Who invented Lewis Dot Structure?

A

Gilbert Lewis

35
Q

What is the NOBLE GAS CONFIGURATION of the Lewis Dot Structure?

A

Duet Rule and the Octet Rule

36
Q

Consists of the element’s symbol surrounding dots to represent the number of valence electrons

A

Lewis Dot Structure

37
Q

What are the 4 Types of Bonding?

A
  1. Ionic Bonding
  2. Covalent Bonding
  3. Metallic Bonding
  4. Intermolecular Forces of Attraction
38
Q
  • Transferring of electrons
  • Metal donates the electron to a non-metal
  • Metal + non-metal
  • Properties of Ionic Compounds
    o Are solid with high melting point ( › 400°C)
    o Conduct electricity when in aqueous solution or in molten state
A

IONIC BONDING

39
Q

Ionic Bonding are soluble in ___.

A

polar solvents

40
Q
  • Sharing of electrons
  • Non-metal + non-metal
    o Single bond (H2O, CH4)
    o Double bond (O2, CO2)
    o Triple bond (N2)
A

Covalent Bonding

41
Q

Properties of Covalent Bonding

A
  1. SLG with low melting points
  2. Soluble in non-polar solvents
42
Q

*Is the force of attraction that holds metals together
*Consists of the attraction of the free-floating valence electrons for the positively charged metal ions
*Explains many physical properties of metals

A

Metallic Bonding

43
Q

*Are the forces of attractions that exist between molecules in a compound
*Cause the compound to exist in solid, liquid, or gas; and affect the melting and boiling points of compounds as well as the solubility of one substance in another

A

Intermolecular Forces of Attraction

44
Q

What is another term of Intermolecular Forces of Attraction?

A

Van der Waals forces (Johannes van der Waals)

45
Q

What are types of Intermolecular Forces of Attraction?

A
  1. Dispersion forces
  2. Dipole to Dipole interaction
  3. Hydrogen Bond
46
Q
  • Weakest of all molecular interactions among non-polar molecules (H2, Cl2)
  • The more electrons that are present in the molecule, the stronger the dispersion forces
A

Dispersion forces

47
Q
  • Occurs between polar molecules
  • The partial positive charge on one molecule is electrostatically attracted to the partial negative charge on a neighboring molecule
A

Dipole to Dipole interaction

48
Q
  • Are the strongest of the intermolecular forces
  • Important in determining the properties of water and biological molecules like protein
  • Occur between molecules from hydrogen being covalently bonded to either fluorine, oxygen or nitrogen
A

Hydrogen Bond

Organic & Inorganic Chemistry (2 decks)

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